For the reaction system A2(g) + B2(g) ⇋ 2AB(g)the equilibrium constant Kc= 2.8A system using this reaction was being tried in a 1.00 L reactor. It was charged with 0.30 mol A2, 0.10 mol B2 and 0.50 mol AB.The system was allowed to come to equilibrium. Which statement below describes the system coming to equilibrium?(Note: in the answers, Q refers to the reaction quotient, K refers to the equilibrium constant).Question 6Select one:a.The reaction goes to the right, more products will form because Q < Kb.The reaction goes to the left, more reactants will form because Q < Kc.The reaction goes to the right, more products will form because Q > Kd.It is not possible to predict in which direction the system will travel to arrive at equilibrium.e.The reaction goes to the left, more reactants will form because Q > K
Question
For the reaction system A2(g) + B2(g) ⇋ 2AB(g)the equilibrium constant Kc= 2.8A system using this reaction was being tried in a 1.00 L reactor. It was charged with 0.30 mol A2, 0.10 mol B2 and 0.50 mol AB.The system was allowed to come to equilibrium. Which statement below describes the system coming to equilibrium?(Note: in the answers, Q refers to the reaction quotient, K refers to the equilibrium constant).Question 6Select one:a.The reaction goes to the right, more products will form because Q < Kb.The reaction goes to the left, more reactants will form because Q < Kc.The reaction goes to the right, more products will form because Q > Kd.It is not possible to predict in which direction the system will travel to arrive at equilibrium.e.The reaction goes to the left, more reactants will form because Q > K
Solution
First, we need to calculate the reaction quotient (Q) to determine the direction in which the reaction will proceed to reach equilibrium. The reaction quotient is given by the expression Q = [AB]^2 / ([A2][B2]), where the brackets denote the molar concentrations of the species.
Given that the initial amounts of A2, B2, and AB are 0.30 mol, 0.10 mol, and 0.50 mol respectively in a 1.00 L reactor, the initial concentrations are 0.30 M, 0.10 M, and 0.50 M respectively.
Substituting these values into the expression for Q gives Q = (0.50)^2 / (0.30 * 0.10) = 0.25 / 0.03 = 8.33.
Comparing Q with the equilibrium constant Kc = 2.8, we see that Q > K. This means that the reaction will proceed to the left to reach equilibrium, forming more reactants. Therefore, the correct answer is e. The reaction goes to the left, more reactants will form because Q > K.
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